Chem 163 Ready for class? Ch1-17 Review
1. What is the temperature…
a) of 15.0g of He sample in 2.0L container at 655Torr?
b) at 3.0atm in 4.00L if the temperature was 530.K at 4.5atm in 1.50L?
2.
O2 (g) + 2 H2 (g)  2 H2O (g)
a) Write the rate expression (with letters k,m,n…)
b) If the reaction is third order for O2 with k = 1.25 1/ (M5 sec), rewrite the rate expression with all
values filled in.
c) What would happen to the rate if the concentration of O2 is doubled? Show your work/logic.
3. List all factors that affects rate of reaction. Briefly explain HOW each factor affects the rate.
4. What is the relationship between bond energy, bond order, bond length?
5.
2 Na(s) + Cl2(g)  2 NaCl (s)
a) Explain Le Chatelier’s principle.
b) What would happen to this reaction when more Cl2 is added to the system?
6. What is the relationship between molecular polarity and vapor pressure? Briefly explain WHY.
7. Sketch a phase diagram. On it label
a) triple pressure
b) super critical fluid
c) sublimation under constant pressure
8. Sketch primitive cubic cell, body centered cubic cell, face centered cubic cell. Label “r” for radius
and “l” for length of cube. For each, write the relationship between r and l (for example, for primitive
cubic cell, you will write l = 2r)
9. A)Define solubility.
b) What happens to the solubility of (g) in (l) with increasing temperature?
10. Draw a sketch showing what osmotic pressure is. Label on the sketch solute, solvent, hypertonic,
hypotonic and semi permeable membrane.
11. Identify acid, base, conjugate acid, conjugate base in
a) HS-(aq) + H2O(l)  S2-(aq) + H3O+(aq)
b) F-(aq) + H2O(l)  HF(aq) + OH-(aq)
12. The rate constant of the reaction is 3.9 × 10-5 M-1s-1. How long (in seconds) is required to decrease
the concentration of A from 1.07 M to 0.24 M?
13. Given the initial rate data for the reaction A + B → C, determine the rate expression (just the
skeleton) for the reaction. Write the rate law with all the values filled in (including k with proper
unit.)
[A], M
[B], M
Initial rate, M/s
0.0460
0.220
1.31  10-4
0.0920
0.220
5.24  10-4
0.0460
0.440
1.31  10-4
14. Write a balanced chemical equation which corresponds to the following equilibrium constant
expression.
PN1/22 PH3/2 2
a)
Kp =
b)
K = [Al3+ ]2 [CO32- ]3
PNH3
15. A) The conjugate base of H2O is ________.
b) The conjugate acid of HPO42- is ________
16. What is the H3O+ concentration of an aqueous solution with a pH of 8.77?
17. Using this data,
2 NO(g) + Cl2(g)
2 NO2(g)
calculate a value for Kc for
2 NO(g) + O2(g)
NOCl(g) + ½ O2(g)
18. For the reaction, 2 SO2(g) + O2(g)
Kc = 3.20 x 10-3
2 NOCl(g)
Kc =
15.5
NO2(g) + ½ Cl2(g)
2 SO3(g), at 450.0 K the equilibrium constant, Kc, has a
value of 4.62. A system was charged to give these initial concentrations: [SO3] = 0.500 M, [O2] =
0.00855 M, [SO2] = 0.254 M. In which direction will it go?
20. A study of the system, 4 NH3(g) + 7 O2(g)
2 N2O4(g) + 6 H2O(g), was carried out. A
system was prepared with [NH3] = [O2] = 3.60 M as the only components initially. At equilibrium,
[N2O4] is 0.60 M. Calculate the equilibrium concentration of O2.
21. 300.mL of 1.50M CaCl2 is mixed with 500.mL of 2.20M Ag2SO4.
(a) Write the chemical equation showing what happens when two solutions are mixed.
(b) How many moles of solid product are produced?
(c) Calculate the concentration of Ca + (aq) .
(d) Calculate the concentration of SO4-2 (aq) .
(e) Calculate the concentration of Cl-1 (aq) .
(f) Calculate the concentration of Ag+1 (aq) .
This is the end of your assignment. The rest is only for your review purpose. However, I
strongly suggest you go over them.
Chem 162 Ready for class? Ch1 -11 Review
1.
What is the concentration in M of
(a) solution made from 42g NaCl in 750.mL solution?
(b) 500.mL solution that is diluted from 60.mL of 5.00M solution?
2.
2 Ag (s) + Mg(NO3)2 (aq)  2 AgNO3 (aq) + Mg (s)
a) What is the oxidizing agent? How can you tell?
b) How many electrons are transferred in this reaction?
c) 40.g of silver would produce how many grams of Mg?
d) If 300. mL of 1.50M Mg(NO3)2 produces 400.mL AgNO3, what is the concentration in M?
e) How many grams of Ag did you start the 86% yield reaction if 100.mL of 1.65M silver nitrate solution
is produced?
3. a) Write metal activity series. Using this write an equation that would
b) replace one metal with another.
c) be predicted as no reaction.
4. Draw the energy diagram (showing reactant and product) for an exothermic reaction. On it, label
reactant, product, activation energy, transition state and H.
5. Write electron configuration for
a) Pb without using core notation
b) Cu with using core notation
c) Co+1
using core notation
6. a)Sketch s, p, and d orbital.
b) ’3p’ is the name of orbital with 3 being ___________ quantum number and p being ___________
quantum number.
c) When drawing box notation, you draw 3 boxes for 3p. Explain why you draw three boxes.
7. a) Draw Lewis Dot structure for CO2.
b) What is the name of hybrid orbital for O?
c) What is the ‘domain’ (electron group) value for C?
c) What is/are the angles around C?
d) Are bonds polar? Explain why/why not.
e) Is CO2 molecule polar? Explain why/why not.
8) Sketch the energy levels showing relative energy levels for n= 1, n=2 … n= infinity.
9. a)How much energy does it take to heat 300.g of water from 15C to 75C?
b) How much energy does it take to heat 300.g of water from 115C to 175C?
10. What is the temperature…
a) of 15.0g of He sample in 2.0L container at 655Torr?
b) at 3.0atm in 4.00L if the temperature was 530.K at 4.5atm in 1.50L?
This is the end of your assignment. The rest is only for your review purpose. However, I
strongly suggest you go over them.
Chem 161 Ready for class? Week 1
1. Sketch a periodic table. On it, label
a) representative elements
b) transition metals
c) halogens
d) alkaline earth metals
e) semi-metals (metalloids)
2. a) List all diatomic molecules.
b) List all elements that are gaseous at room temperature.
c) List all elements that are liquid at room temperature.
d) Using the information above, write a balanced equation for
I) Nitrogen reaction with oxygen to make dinitrogen pentoxide (g).
II) Making water from ‘scratch’.
III) Decomposition of MgO(s) .
3 . What is the formula of a compound with
a) sodium and chlorine?
What is the name of this compound?
b) magnesium and sulfur?
What is the name of this compound?
C) nitrate and aluminum?
What is the name of this compound?
d) sulfate and hydrogen?
What is the name of this compound?
3. A) Is density intensive or extensive property?
b) What does it mean to be intensive?
c) Name two other properties that are intensive.
4. There are 4 significant figures in 0.04102cm with the estimation in 2, and it means anywhere
between 0.04101cm to 0.04103cm. Answer the following using this example.
a) There are ____ significant figures in 12.50g with the estimation in ________ , and it means
anywhere between ________________________.
b) There are ____ significant figures in 100 g with the estimation in ________ , and it means
anywhere between ________________________.
c) There are ____ significant figures in 100. g with the estimation in ________ , and it means
anywhere between ________________________.
5. A) Briefly state the significant figure rules when adding or subtracting. Show an example.
b) Briefly state the significant figure rules when multiplying or dividing. Show an example.
6. Give three examples of
a) element
b) molecular compound
c) cation
d) ionic compound
7. A) If you have to ‘mix’ hydrogen and oxygen to make H2O, why is H2O considered a compound, not a
mixture?
b) Both hydrogen and oxygen are diatomic and should be written as H2 and O2. If this is the case, why
is water H2O? Not H2O2?
8. Each ‘box’ of the periodic table has three information. The whole number on top is called
________________ and the decimal number on the bottom is called ________________ with the unit
of ________________.
9. (a) Mole (mol) is a name given for the number 6.022x1023. If you have 2 mol water molecules, it
means you have _________________ water molecules. However if you are counting elements, there
are ________________ elements since each water molecule has ___ elements.
b) Mole (mol) is a name given for the number 6.022x1023. If you have 5 mol Ca(OH)2, it means you have
______________________ Ca(OH)2. However if you are counting ions, there are
________________ ions since each Ca(OH)2 has ___ ions, and if you are counting just the anions, there
are _______________anions since each Ca(OH)2 has ____ anions.
10. (a) One the average, 6.022 x 1023 helium weigh 4.0g. We may write this as ( 4.0g / 6.022 x 1023
helium ) or (4.0g / 1 mol He ). Using this, you can say 3 mol He weighs _______ g, and 40.g of He is
equivalent to _____ mol of He.
(b) One the average, 6.022 x 1023 oxygen gas weigh 32 g . We may write this as ( 32g / 6.022 x 1023
O2 ) or (32g / 1 mol O2 ). Using this, you can say 4.5 mol O2 weight _______ g and 97g of O2 is
equivalent to _______ mol O2.
11. What is the molar mass for (please include unit!)
a) ammonium phosphate?
b) carbonic acid?
b) nitrogen gas?
12.
P4 (s)
+
10 Cl2 (g)

4 PCl5 (g)
a) This equation reads, 1 molecule of P4 react with 10 molecules of Cl2 to produce 4 molecules of PCl5.
How many molecules of Cl2 do you need to react with 5 molecules of P4? Clearly show your work.
b) This equation reads, 6.22x1023 (1mol) molecule of P4 react with 6.22x1024 (10 mol) molecules of Cl2 to
produce 2.4088x1023 (4mol) molecules of PCl5.
6.0mol of of Cl2? Clearly show your work.
How many mole of PCl5 would be produced from
c) How many grams of product would you get from 350.g of Cl2? Show your work clearly!!
d) What is the amount of P4 (s) that you had to ASSUME to have in (C)?
e) Are you calculating the ‘theoretical’ or ‘actual” yield in (c)?
13. You have two solutions : 500.mL of 2.0M NaCl and 500mL of 2.0M CO2.
a)
Is NaCl an ionic compound or a molecular compound?. Explain your answer.
b) Is CO2 an ionic compound or a molecular compound?. Explain your answer.
c) Calculate the number of moles of NaCl in 500.mL of 2.0M NaCl.
d) Calculate the number of moles of CO2 in 500mL of 2.0M CO2.
e) What type of compound is NaCl? What type of compound is CO2?
f) Calculate the number of moles of “things” in 500.mL of 2.0M NaCl. Think about what is
actually present in water. Is it NaCl? Na and Cl? Na+ and Cl-? Na and Cl2?...
g) Calculate the number of moles of “things” in 500mL of 2.0M CO2. Think about what is actually
present in water. Is it CO2? C and O? C and O2?.....
Chem 161 Ready for class? Ch1 to 4 Review
1. Sketch a periodic table. On it, label
a) representative elements
b) transition metals
c) halogens
d) alkaline earth metals
e) semi-metals (metalloids)
2. a) List all diatomic molecules.
b) List all elements that are gaseous at room temperature.
c) List all elements that are liquid at room temperature.
d) Using the information above, write a balanced equation for
I) Nitrogen reaction with oxygen to make dinitrogen pentoxide (g).
II) Making water from ‘scratch’.
III) Decomposition of MgO(s) .
3 . What is the formula of a compound with
a) sodium and chlorine?
What is the name of this compound?
b) magnesium and sulfur?
What is the name of this compound?
C) nitrate and aluminum?
What is the name of this compound?
d) sulfate and hydrogen?
What is the name of this compound?
3. A) Is density intensive or extensive property?
b) What does it mean to be intensive?
c) Name two other properties that are intensive.
4. There are 4 significant figures in 0.04102cm with the estimation in 2, and it means anywhere
between 0.04101cm to 0.04103cm. Answer the following using this example.
a) There are ____ significant figures in 12.50g with the estimation in ________ , and it means
anywhere between ________________________.
b) There are ____ significant figures in 100 g with the estimation in ________ , and it means
anywhere between ________________________.
c) There are ____ significant figures in 100. g with the estimation in ________ , and it means
anywhere between ________________________.
5. A) Briefly state the significant figure rules when adding or subtracting. Show an example.
b) Briefly state the significant figure rules when multiplying or dividing. Show an example.
6. Give three examples of
a) element
b) molecular compound
c) cation
d) ionic compound
7. A) If you have to ‘mix’ hydrogen and oxygen to make H2O, why is H2O considered a compound, not a
mixture?
b) Both hydrogen and oxygen are diatomic and should be written as H2 and O2. If this is the case, why
is water H2O? Not H2O2?
8. Each ‘box’ of the periodic table has three information. The whole number on top is called
________________ and the decimal number on the bottom is called ________________ with the unit
of ________________.
9. (a) Mole (mol) is a name given for the number 6.022x1023. If you have 2 mol water molecules, it
means you have _________________ water molecules. However if you are counting elements, there
are ________________ elements since each water molecule has ___ elements.
b) Mole (mol) is a name given for the number 6.022x1023. If you have 5 mol Ca(OH)2, it means you have
______________________ Ca(OH)2. However if you are counting ions, there are
________________ ions since each Ca(OH)2 has ___ ions, and if you are counting just the anions, there
are _______________anions since each Ca(OH)2 has ____ anions.
10. (a) One the average, 6.022 x 1023 helium weigh 4.0g. We may write this as ( 4.0g / 6.022 x 1023
helium ) or (4.0g / 1 mol He ). Using this, you can say 3 mol He weighs _______ g, and 40.g of He is
equivalent to _____ mol of He.
(b) One the average, 6.022 x 1023 oxygen gas weigh 32 g . We may write this as ( 32g / 6.022 x 1023
O2 ) or (32g / 1 mol O2 ). Using this, you can say 4.5 mol O2 weight _______ g and 97g of O2 is
equivalent to _______ mol O2.
11. What is the molar mass for (please include unit!)
a) ammonium phosphate?
b) carbonic acid?
b) nitrogen gas?
12.
P4 (s)
+
10 Cl2 (g)

4 PCl5 (g)
a) This equation reads, 1 molecule of P4 react with 10 molecules of Cl2 to produce 4 molecules of PCl5.
How many molecules of Cl2 do you need to react with 5 molecules of P4? Clearly show your work.
b) This equation reads, 6.22x1023 (1mol) molecule of P4 react with 6.22x1024 (10 mol) molecules of Cl2 to
produce 2.4088x1023 (4mol) molecules of PCl5.
How many mole of PCl5 would be produced from
6.0mol of of Cl2? Clearly show your work.
c) How many grams of product would you get from 350.g of Cl2? Show your work clearly!!
d) What is the amount of P4 (s) that you had to ASSUME to have in (C)?
e) Are you calculating the ‘theoretical’ or ‘actual” yield in (c)?
13. You have two solutions : 500.mL of 2.0M NaCl and 500mL of 2.0M CO2.
a)
Is NaCl an ionic compound or a molecular compound?. Explain your answer.
b) Is CO2 an ionic compound or a molecular compound?. Explain your answer.
c) Calculate the number of moles of NaCl in 500.mL of 2.0M NaCl.
d) Calculate the number of moles of CO2 in 500mL of 2.0M CO2.
e) What type of compound is NaCl? What type of compound is CO2?
f) Calculate the number of moles of “things” in 500.mL of 2.0M NaCl. Think about what is
actually present in water. Is it NaCl? Na and Cl? Na+ and Cl-? Na and Cl2?...
g) Calculate the number of moles of “things” in 500mL of 2.0M CO2. Think about what is actually
present in water. Is it CO2? C and O? C and O2?.....
14. How many mL of 0.446 M KMnO4(aq) are required to react with 50.0 mL of 0.200 M H2C2O4(aq) ?
2 KMnO4(aq) + 5 H2C2O4(aq) + 3 H2SO4(aq)
15 . Assign oxidation number for…
 2 MnSO4(aq) + 10 CO2(g) + 8 H2O + K2SO4(aq)
Show your work/logic.
a) Mn in KMnO4
b) C in C3H8O
c) vanadium in (NH4)3VO4
d) carbon in K2C2O4
e) boron in Na2B4O7
16. Identify each reaction to be oxidation, reduction, redox, or non-redox. Show your work/logic.
a.
Ba2+(aq) + CrO42-(aq)  BaCrO4(s)
b.
2 H+(aq) + CO32-(aq)  H2O(l) + CO2(g)
c.
Fe3+(aq)
d.
MnO2(s)  MnO4-(aq)
e.
2 CrO42-(aq) + 2 H+(aq)  Cr2O72-(aq) + H2O(l)

Fe2+(aq)
17. The following reaction describes the production of metallic iron: 2Fe2O3 + 3C  4Fe + 3CO2
How many electrons are lost by each carbon atom in this reaction? Show your work/logic.
18. Consider the redox equation, C4H10(l) + Cr2O72-(aq) + H+(aq)  H6C4O4(s) + Cr3+(aq) +
H2O(l)
The oxidizing agent is …
19. The activity series of metals is
Au < Ag < Cu < Sn < Cd < Zn < Al < Mg < Na < Cs
list, which element would undergo oxidation most readily?
Based on this
20. Using the activity series given above, predict the products or predict ‘no reaction.
a)
Al+3 (aq) +
Mg(s)

b)
Al(s)
+ Mg+2(aq) 
c)
AlCl3 (aq) + Mg(s) 
d)
Al(s) + MgCl2 (aq) 
e)
Compare reactions (a) and (b).
f)
Compare reactions (a) and (c).
g)
Compare reactions (b) and (d).
21. When the carbohydrate, C12H22O11, undergoes complete combustion (products are CO2 and water),
a)
write a balanced equation
b)
Above the balanced equation, assign oxidation number for EACH atom of each element in the
equation.
c)
the reducing agent in the reaction is…
22. When the carbohydrate, C12H22O11, undergoes incomplete combustion (products are CO and water),
a)
write a balanced equation
b)
the reducing agent in the reaction is..
c)
Compare these answers to question above and explain the condition that might lead to
incomplete combustion.
23. BrO3-(aq) + Zn(s) +  Br-(aq) + Zn2+(aq)
a) Assign oxidation numbers for each element. Be clear.
b) Reducing agent?
c) Oxidizing agnet?
d) How many electrons do you think should be transferred once balanced correctly? Show your
work/logic. Figure it out without balancing the whole equation.
24. C4H10(l) + Cr2O72-(aq) + H+(aq)  H6C4O4(s) + Cr3+(aq) + H2O(l)
a)
Assign oxidation numbers for each element. Be clear.
b)
Reducing agent?
c)
Oxidizing agnet?
d)
How many electrons do you think should be transferred once balanced correctly? Show your
work/logic. Figure it out without balancing the whole equation.